Molarity • Tostudysolutionstoichiometry,wemustknowhowmuchofthereactantsarepresentinasolutionandalsohowtocontroltheamountsofreactantsusedtobringaboutareactioninaqueoussolution
• Concentration=theamountofsolutepresentinagivenamountofsolvent,oragivenamountofsolution
• Insolutionstoichiometry,weusetheconcentrationasaconversionbetweenamount(volume,g)andmolesofasubstanceinsolution
Molarity • Topreparesolutionsofknownconcentration,youwould:
① Massthesolid② Placeinavolumetricflaskofappropriatevolume③ Addenoughdistilledwatertodissolvethesolid④ THENaddwatertothespecifiedmarkontheflask*Ifyoudumpthesolidintotheentirevolumeofwater,
youareneglectingthespacethesolidwilloccupyandyoursolutionwillnotmatchyourconcentration*
Molarity • StandardSolution=Asolutionwhoseconcentrationisaccuratelyknown– Volumetricflask–containsanexacttotalvolumeofsolution
Molarity • Ex/Calculatethemolarityofasolutionpreparedbydissolving11.5gofsolidNaOHinenoughwatertomake1.50Lofsolution
Molarity • Ex/Calculatethemolarityofasolutionpreparedbydissolving1.56gofgaseousHClinenoughwatertomake26.8mLofsolution
Molarity • Usebalanceddissociationequationtodeterminetheconcentrationofindividualions
• Inotherwords,wearebasicallymultiplyingionsbytheirsubscript/coefficient
• Ex/Givetheconcentrationofeachtypeofionin0.50MCo(NO3)2
Molarity • Usemolaritytoconvertbetweenmolesandliters• Ex/CalculatethenumberofmolesofCl-ionsin1.75Lof1.0x10-3MZnCl2
Dilution• Concentratedsolutionsareoftenusedas“stock”solutions
• Thesecanbedilutedtopreparealessconcentratedsolution
Dilution• Equipmentinvolved:
– Pipet/Pipette–toaccuratelymeasureandtransferagivenvolumeofsolution.Maybemeasuring(gradation)orvolumetric(onlyasinglemeasurementvalue)
Dilution• Ex/Describehowyouwouldprepare5.00x102mLofa1.75MH2SO4solution,startingwithan8.61MH2SO4stocksolution
First:M1= M2=V1= V2=
Dilution• Ex/Describehowyouwouldprepare5.00x102mLofa1.75MH2SO4solution,startingwithan8.61MH2SO4stocksolution
First:M1=8.61M M2=1.75MV1=? V2=5.00x102mLSecond:PlugintoM1V1=M2V2
Third:Howdoyoupreparethenewconcentration?
PrecipitationReactions• Precipitationreactionsoccurinaqueoussolutionandresultintheformationofaninsolubleproduct(precipitate)
• Ex/Pb(NO3)2(aq)+2KI(aq)àPbI2(s)+2KNO3(aq)
PrecipitationReactions• Weoftenseparatetheprecipitatefromthesolutionbyfiltrationusinggravimetricanalysis(moreonthismomentarily)
PrecipitationReactions• SolubilityRulesàmemorizethecommononesØ MostalkalimetalsaltsandNH4
+saltsaresolubleØ Cl-,Br-,I-aresoluble(exceptforAg+,Hg22+,Pb2+)Ø F-aresoluble(exceptforIIAmetals)Ø NO3
-,ClO3-,ClO4
-,andCH3COO-aresolubleØ SO4
2-aresoluble(exceptforCa,Sr,Ba,Ag+,Pb2+,Hg22+)
Ø CO32-,PO4
3-,C2O42-,CrO4
2-,S2-,OH-,andO2-areinsoluble(exceptforcaseswithrule#1)
Ø Itcanbeassumedthatsaltsthatdissolveinwaterarestrongelectrolytes
PrecipitationReactions• Wecanpredictwhetherornotprecipitateswillformusingsolubilityrules
• Ex/Whatprecipitate(ifany)willformifthefollowingpairsofsolutionsaremixed?a. KNO3andBaCl2b. Na2SO4andPb(NO3)2c. KOHandFe(NO3)3
RxnsinSoln’s• Wecandescribereactionsinsolutionsafewdifferentways:
§ Completebalancedequation• Thisistheoverallreaction
§ Completeionicequation• Thisrepresentsallsolublecompounds/electrolytesasions
§ Netionicequations• Spectatorions(ionsthatdidnotchangeorwerenotinvolved)areexcludedandonlythosesolutioncomponentsundergoingachangeareincluded
PrecipitationReactions• Ex/Whatprecipitate(ifany)willformifthefollowingpairsofsolutionsaremixed?a. KNO3andBaCl2b. Na2SO4andPb(NO3)2c. KOHandFe(NO3)3
GravimetricAnalysis• Gravimetricanalysis=analyticaltechniqueusedtodeterminetheconcentrationofananalyte(anionbeinganalyzed)byprecipitatingtheionasaninsolublesalt,whichcanthenbemassed
GravimetricAnalysis• Typically,itinvolvestheformation,isolation,andmassdeterminationofaprecipitate
1. Determinetheanalyte/ionyouneedtoprecipitate2. Chooseareactionthatwillproduceaninsolublesalt
thatcontainsthation3. Performaprecipitationrxntocompletelyprecipitate
thetargetionàbesuretoaddexcessoftheothersolutiontoensurecompleteprecipitation(otherwiseyourconcentrationwillbeinaccurate)
4. Carefully,filter,wash,anddrytheprecipitate5. Takethemass6. Usestoichiometrytofigureoutyourconcentration
GravimetricAnalysis• Ex/Astudentwantstodetermine[Ba+2]in100.00mLofanunknownsolutionofBa+2.Shedecidedtoprecipitatethebariumionsasbariumsulfate,aninsolublesalt.Sheaddsanexcessofsodiumsulfatesolutiontothebariumsolutionuntilnomoreprecipitateforms.Shethenfilters,washes,anddriestheprecipitate.Shemeasuresthemasstobe2.917g.Determine[Ba+2]inthesolution.
GravimetricAnalysis• First,assembleyourknowninformation• Vsoln=100.00mL MassBaSO4=2.917g• Second,writeyourbalancednetionicequation:
Ba2+(aq)+SO42-(aq)àBaSO4(s)
• Third,usestoichiometrytodeterminethemolofyouranalyte(Ba2+)
• Lastly,dividebyvolumeofyoursolutiontogetmolarity
GravimetricAnalysis• Filters,washes,anddriestheppt,andmeasuresitsmasstobe2.917g
• Writetheequation:• Ba+2(aq)+SO4
2-(aq)àBaSO4(s)
• Makesuretheequationisbalanced• Convert2.917gBaSO4tomolofBa2+
• Dividebythevolumeofsolutiontogettheconcentration
GravimetricAnalysis• Trythis:• 25.00mLofalead(II)nitratesolutionistreatedwithexcessaqueoussodiumsulfate.Afterfiltrationanddrying,0.303gofsolidleadsulfateisisolated.Whatwastheconcentrationofthelead(II)nitratesolution?
GravimetricAnalysis• Trythis:A0.5662-gsampleofanioniccompoundcontainingchlorideionsandanunknownmetalisdissolvedinwaterandtreatedwithanexcessofAgNO3.If1.0882gofAgClprecipitateforms,whatisthepercentbymassoftheoriginalcompound?
• Hint,%Cl=massofCl/0.5662gsamplex100%